Consider the following plots of rate constant versus `(1)/(T)` for four different reactions. Which of the following orders is correct for the activation energies of these reactions?

Options

A. `E_(b) gt E_(d) gt E_(c)gt E_(a)`
B. `E_(a) gt E_(c) gt E_(d) gt E_(b)`
C. `E_(b) gt E_(a) gt E_(d) gt E_(c)`
D. `E_(c) gt E_(a) gt E_(d) gt E_(b)`

Answer

D

Explanation

`k=Ae^(-Ea//RT)`
log k = log `A-(E_(a))/(2.303 RT)," slope "=(-E_(a))/(2.303 R)`
`therefore` In the given graph, greater the slope, more is the `E_(a)`
`therefore "Order "=E_(c) gt E_(a) gt E_(d) gt E_(b)`